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MIT 5.111 Principles of Chemical Science, Fall 2008

by: MIT OpenCourseWare

Publication date: 2008
Usage: Attribution-Noncommercial-Share Alike 3.0
Topics: introductory chemistry, atomic structure, molecular electronic structure, thermodynamics, acid-base equillibrium, titration, redox, chemical kinetics, catalysis, lewis structures, VSEPR theory, wave-particle duality, biochemistry, orbitals, periodic trends, general chemistry, valence bond theory, hybridization, free energy, reaction mechanism, Rutherford backscattering
Language: English
Item Size: 10.4G

The MIT 5.111 Principles of Chemical Science, Fall 2008 course provides an introduction to the chemistry of biological, inorganic, and organic molecules. The emphasis is on basic principles of atomic and molecular electronic structure, thermodynamics, acid-base and redox equilibria, chemical kinetics, and catalysis.

Instructors: Prof. Catherine Drennan, Dr. Elizabeth Vogel Taylor

View the complete course at: http://ocw.mit.edu/5-111F08

License: Creative Commons BY-NC-SA

More information at http://ocw.mit.edu/terms

More courses at http://ocw.mit.edu

Addeddate: 2009-07-02 18:22:53
Color: color
Identifier: MIT5.111F08
Sound: sound
Year: 2008

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MPEG4

60.8M

Lecture 01: The importance of chemical principles

103.2M

Lecture 02: Discovery of electron and nucleus, need for quantum mechanics

106.6M

Lecture 03: Wave-particle duality of light

99.3M

Lecture 04: Wave-particle duality of matter, Schrödinger equation

105.1M

Lecture 05: Hydrogen atom energy levels

106.2M

Lecture 06: Hydrogen atom wavefunctions (orbitals)

103.5M

Lecture 07: p-orbitals

108.6M

Lecture 08: Multielectron atoms and electron configurations

110.2M

Lecture 09: Periodic trends

105.5M

Lecture 10: Periodic trends continued; Covalent bonds

112.2M

Lecture 11: Lewis structures

111.1M

Lecture 12: Exceptions to Lewis structure rules; Ionic bonds

99.1M

Lecture 13: Polar covalent bonds; VSEPR theory

112.9M

Lecture 14: Molecular orbital theory

90.5M

Lecture 15: Valence bond theory and hybridization

111.3M

Lecture 16: Determining hybridization in complex molecules; Thermochemistry and bond energies/bond enthalpies

106.8M

Lecture 17: Entropy and disorder

98.1M

Lecture 18: Free energy and control of spontaneity

100.9M

Lecture 19: Chemical equilibrium

110.1M

Lecture 20: Le Chatelier's principle and applications to blood-oxygen levels

81.5M

Lecture 21: Acid-base equilibrium: Is MIT water safe to drink?

110.6M

Lecture 22: Chemical and biological buffers

100.3M

Lecture 23: Acid-base titrations

104.7M

Lecture 24: Balancing oxidation/reduction equations

106.6M

Lecture 25: Electrochemical cells

102.9M

Lecture 26: Chemical and biological oxidation/reduction reactions

98.5M

Lecture 27: Transition metals and the treatment of lead poisoning

99.8M

Lecture 28: Crystal field theory

92.6M

Lecture 29: Metals in biology

85.4M

Lecture 30: Magnetism and spectrochemical theory

93.9M

Lecture 31: Rate laws

98.5M

Lecture 32: Nuclear chemistry and elementary reactions

100.1M

Lecture 33: Reaction mechanism

92.6M

Lecture 34: Temperature and kinetics

106.2M

Lecture 35: Enzyme catalysis

68.9M

Lecture 36: Biochemistry

OGG VIDEO

117.5M

Lecture 01: The importance of chemical principles

200.9M

Lecture 02: Discovery of electron and nucleus, need for quantum mechanics

207.2M

Lecture 03: Wave-particle duality of light

192.6M

Lecture 04: Wave-particle duality of matter, Schrödinger equation

204.0M

Lecture 05: Hydrogen atom energy levels

206.6M

Lecture 06: Hydrogen atom wavefunctions (orbitals)

201.1M

Lecture 07: p-orbitals

210.6M

Lecture 08: Multielectron atoms and electron configurations

213.5M

Lecture 09: Periodic trends

204.9M

Lecture 10: Periodic trends continued; Covalent bonds

217.6M

Lecture 11: Lewis structures

215.2M

Lecture 12: Exceptions to Lewis structure rules; Ionic bonds

191.7M

Lecture 13: Polar covalent bonds; VSEPR theory

219.2M

Lecture 14: Molecular orbital theory

175.4M

Lecture 15: Valence bond theory and hybridization

215.8M

Lecture 16: Determining hybridization in complex molecules; Thermochemistry and bond energies/bond enthalpies

207.9M

Lecture 17: Entropy and disorder

190.5M

Lecture 18: Free energy and control of spontaneity

195.9M

Lecture 19: Chemical equilibrium

213.3M

Lecture 20: Le Chatelier's principle and applications to blood-oxygen levels

156.9M

Lecture 21: Acid-base equilibrium: Is MIT water safe to drink?

213.7M

Lecture 22: Chemical and biological buffers

193.2M

Lecture 23: Acid-base titrations

202.5M

Lecture 24: Balancing oxidation/reduction equations

206.5M

Lecture 25: Electrochemical cells

198.4M

Lecture 26: Chemical and biological oxidation/reduction reactions

191.6M

Lecture 27: Transition metals and the treatment of lead poisoning

193.3M

Lecture 28: Crystal field theory

179.9M

Lecture 29: Metals in biology

166.5M

Lecture 30: Magnetism and spectrochemical theory

181.6M

Lecture 31: Rate laws

191.6M

Lecture 32: Nuclear chemistry and elementary reactions

194.1M

Lecture 33: Reaction mechanism

179.3M

Lecture 34: Temperature and kinetics

204.5M

Lecture 35: Enzyme catalysis

133.7M

Lecture 36: Biochemistry

SUBRIP

42.9K

Lecture 01: The importance of chemical principles

66.2K

Lecture 02: Discovery of electron and nucleus, need for quantum mechanics

68.9K

Lecture 03: Wave-particle duality of light

62.5K

Lecture 04: Wave-particle duality of matter, Schrödinger equation

65.0K

Lecture 05: Hydrogen atom energy levels

68.2K

Lecture 06: Hydrogen atom wavefunctions (orbitals)

66.9K

Lecture 07: p-orbitals

72.6K

Lecture 08: Multielectron atoms and electron configurations

76.7K

Lecture 09: Periodic trends

73.0K

Lecture 10: Periodic trends continued; Covalent bonds

78.1K

Lecture 11: Lewis structures

75.0K

Lecture 12: Exceptions to Lewis structure rules; Ionic bonds

66.5K

Lecture 13: Polar covalent bonds; VSEPR theory

73.2K

Lecture 14: Molecular orbital theory

57.7K

Lecture 15: Valence bond theory and hybridization

72.8K

Lecture 16: Determining hybridization in complex molecules; Thermochemistry and bond energies/bond enthalpies

69.6K

Lecture 17: Entropy and disorder

66.7K

Lecture 18: Free energy and control of spontaneity

49.0K

Lecture 19: Chemical equilibrium

57.1K

Lecture 20: Le Chatelier's principle and applications to blood-oxygen levels

37.8K

Lecture 21: Acid-base equilibrium: Is MIT water safe to drink?

56.4K

Lecture 22: Chemical and biological buffers

53.9K

Lecture 23: Acid-base titrations

54.7K

Lecture 24: Balancing oxidation/reduction equations

53.7K

Lecture 25: Electrochemical cells

51.5K

Lecture 26: Chemical and biological oxidation/reduction reactions

49.7K

Lecture 27: Transition metals and the treatment of lead poisoning

45.0K

Lecture 28: Crystal field theory

41.1K

Lecture 29: Metals in biology

40.8K

Lecture 30: Magnetism and spectrochemical theory

44.2K

Lecture 31: Rate laws

50.1K

Lecture 32: Nuclear chemistry and elementary reactions

47.0K

Lecture 33: Reaction mechanism

50.4K

Lecture 34: Temperature and kinetics

56.4K

Lecture 35: Enzyme catalysis

33.6K

Lecture 36: Biochemistry

TORRENT

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